Question 1

Calculate the solubility product of calcium hydroxide given that the solubility of Ca(OH)2(s) in water at 25S1U1P1$\circ$S1S1P0C is 0.011 M.

Accepted Answer

A)  1.5 * 10-8  
B)  1.1 * 10-5  
C)  2.7 * 10-6  
D)  5.3 * 10-6  
E)  1.2 * 10-4  
A)  1.5 * 10-8  
B)  1.1 * 10-5  
C)  2.7 * 10-6  
D)  5.3 * 10-6  
E)  1.2 * 10-4

Question 2

Choose the effective pH range of a HF/NaF buffer.For HF,Ka = 3.5 * 10-4.

Accepted Answer

A)  6.0-8.0 
B)  9.6-11.6 
C)  5.0-7.0 
D)  0.7-2.7 
E)  2.5-4.5 
A)  6.0-8.0 
B)  9.6-11.6 
C)  5.0-7.0 
D)  0.7-2.7 
E)  2.5-4.5

Question 3

Given the half reaction: NO3-(aq) $\rightarrow$NO(g),In acidic solution,How many electrons appear in the half-reaction when it is properly balanced?

Accepted Answer

A)  3 
B)  4 
C)  6 
D)  8 
E)  None of the above. 
A)  3 
B)  4 
C)  6 
D)  8 
E)  None of the above.

Question 4

The standard potential of the cell
Pb(s)|PbSO4(s)|SO42-(aq)M Pb2+(aq)|Pb(s)
Is +0.23 V at 25$\omicron$C.Calculate the Ksp of PbSO4.

Accepted Answer

A)  1.3 *10-18  
B)  1.7 * 10-8  
C)  1.3 * 10-4  
D)  2.7 * 10-17  
E)  6.0 * 107  
A)  1.3 *10-18  
B)  1.7 * 10-8  
C)  1.3 * 10-4  
D)  2.7 * 10-17  
E)  6.0 * 107

Question 5

The following 0.1 M aqueous solutions are arranged in order of increasing pH, with the highest pH on the far right. $$\begin{array} { | l | l | l | l | l | } 
\hline \mathrm { C } _ { 5 } \mathrm { H } _ { 5 } \mathrm { NHCl } & \mathrm { HClO } & \mathrm { KNO } _ { 3 } & \mathrm { NaClO } & \
\hline
\end{array}$$
Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Accepted Answer

A)  NaCN 
B)  CH3COOH 
C)  KNO2  
D)  NaBr 
E)  NaHSO4  
A)  NaCN 
B)  CH3COOH 
C)  KNO2  
D)  NaBr 
E)  NaHSO4

Question 6

What are the products of the electrolytic reduction of copper from aqueous CuSO4?

Accepted Answer

A)  H2(g) and H2SO3(aq). 
B)  Cu(s) and O2(g). 
C)  H2SO3(aq) and O2(g). 
D)  Cu(s) and H2SO3(aq). 
E)  H2(g) and O2(g). 
A)  H2(g) and H2SO3(aq). 
B)  Cu(s) and O2(g). 
C)  H2SO3(aq) and O2(g). 
D)  Cu(s) and H2SO3(aq). 
E)  H2(g) and O2(g).

Question 7

In liquid ammonia,the acid HB is a strong acid if it is a weaker proton donor than NH4+.

Accepted Answer

A) True 
 B)False

Question 8

The boxes below contain a series of 0.1 M aqueous solutions of increasing pH where A is the solution of lowest pH and E is the solution of highest pH. $$\begin{array} { | c | c | c | c | c | } 
\hline \mathrm { A } & \mathrm { B } & \mathrm { C } & \mathrm { D } & \mathrm { E } \
\hline
\end{array}$$ 
Match each box with the correct compound.
phenol,pKa = 9.89
cyanide ion,pKb = 4.69
pyridine,pKb = 8.75
hydrogen sulfate ion,pKa = 1.92
sodium nitrate

Accepted Answer

phenol,pK_a = 9.89 (B) cyanide i

Question 9

A solution is prepared by mixing equal volumes of 0.40 M HF(aq)with 0.40 M KOH(aq).This solution is a buffer.

Accepted Answer

A) True 
 B)False

Question 10

You have available the following reagents as 0.10 M aqueous solutions: NaOH, HCl,HCN (pKa = 9.31),Aniline (pKb = 9.13),HNO2 (pKa = 3.25),And CH3NH2 (pKb = 3.34).Which two reagents would you use to make a buffer with a pH of 10.6?

Accepted Answer

A)  NaOH and HCN 
B)  HCl and aniline 
C)  HCl and CH3NH2 
D)  NaOH and HNO2 
A)  NaOH and HCN 
B)  HCl and aniline 
C)  HCl and CH3NH2 
D)  NaOH and HNO2

Question 11

The pH of 0.010 M H3PO4(aq) is 2.24.Estimate the concentration of HPO42- in the solution.For H3PO4,The values of Ka1,Ka2,And Ka3 are 7.6 * 10-3,6.2 * 10-8,And 2.1 * 10-13,Respectively.

Accepted Answer

A)  5.8 * 10-3 M 
B)  7.6 * 10-3 M 
C)  0.010 M 
D)  6.2 * 10-8 M 
E)  2.1 *10-13 M 
A)  5.8 * 10-3 M 
B)  7.6 * 10-3 M 
C)  0.010 M 
D)  6.2 * 10-8 M 
E)  2.1 *10-13 M

Question 12

Estimate the pH of 0.10 M Na2HPO4(aq) given pKa1 = 2.12,
PKa2 = 7.21,And pKa3 = 12.68 for phosphoric acid.

Accepted Answer

A)  12.68 
B)  9.94 
C)  7.40 
D)  4.67 
E)  2.12 
A)  12.68 
B)  9.94 
C)  7.40 
D)  4.67 
E)  2.12

Question 13

Calculate the [OH-] in an aqueous solution that is 0.125 M NH3 and 0.300 M NH4Cl .The value of Kb for NH3 is 1.8 * 10-5.

Accepted Answer

A)  0.425 M 
B)  0.125 M 
C)  1.8 * 10-5 M 
D)  7.5 * 10-6 M 
E)  4.3 *10-5 M 
A)  0.425 M 
B)  0.125 M 
C)  1.8 * 10-5 M 
D)  7.5 * 10-6 M 
E)  4.3 *10-5 M

Question 14

The Ka of phenol is 1.3 * 10-10 .For a solution labeled "1.0 * 10-3 M aqueous phenol,"

Accepted Answer

A)  [H3O+] = [H3O+]2/[phenol]initial. 
B)  [H3O+] initial. 
C)  [H3O+] > 10 -6. 
D)  pH ~ 4. 
E)  Kw/[H3O+] >> [phenol]initial. 
A)  [H3O+] = [H3O+]2/[phenol]initial. 
B)  [H3O+] initial. 
C)  [H3O+] > 10 -6. 
D)  pH ~ 4. 
E)  Kw/[H3O+] >> [phenol]initial.

Question 15

What is the equilibrium constant for the titration reaction involving CH3NH2(aq) and HBr(aq)?

Accepted Answer

A)  1.0 * 1014 
B)  2.8 * 103 
C)  2.8 * 10-11 
D)  3.6 * 1010 
A)  1.0 * 1014 
B)  2.8 * 103 
C)  2.8 * 10-11 
D)  3.6 * 1010

Question 16

If equal volumes of 0.004 M Pb(NO3)2(aq) and 0.004 M KI(aq) Are mixed,What reaction,If any,Occurs? The value of Ksp for PbI2 is 1.4 * 10-8.

Accepted Answer

A)  The solution turns purple because of formation of I2. 
B)  PbI2(s) precipitates. 
C)  KNO3(s) precipitates. 
D)  No reaction occurs. 
E)  The value of Ksp changes to 9 * 10-9.  
A)  The solution turns purple because of formation of I2. 
B)  PbI2(s) precipitates. 
C)  KNO3(s) precipitates. 
D)  No reaction occurs. 
E)  The value of Ksp changes to 9 * 10-9.

Question 17

Silver bromide is most soluble in

Accepted Answer

A)  pure H2O(l). 
B)  dilute HNO3(aq). 
C)  0.10 M AgNO3(aq). 
D)  dilute NH3(aq). 
E)  0.10 M NaCl(aq). 
A)  pure H2O(l). 
B)  dilute HNO3(aq). 
C)  0.10 M AgNO3(aq). 
D)  dilute NH3(aq). 
E)  0.10 M NaCl(aq).

Question 18

Calculate the [OH-] in an aqueous solution that is 0.125 M NH3 and 0.125 M NH4Cl .The value of Kb for NH3 is 1.8 * 10 -5.

Accepted Answer

A)  1.8 * 10-5 M 
B)  5.5 * 10-10 M 
C)  6.7 * 10-12 M 
D)  0.125 M 
E)  1.5 *10-3 M 
A)  1.8 * 10-5 M 
B)  5.5 * 10-10 M 
C)  6.7 * 10-12 M 
D)  0.125 M 
E)  1.5 *10-3 M

Question 19

A cell that uses bromine to oxidize hydrogen to H+ under standard conditions at 298 K has a negative potential?

Accepted Answer

A) True 
 B)False

Question 20

For the cell diagram
Pt|H2(g),H+(aq)M Cu2+(aq)|Cu(s)
Which reaction occurs at the anode?

Accepted Answer

A)  Cu(s) $\rightarrow$Cu2+(aq) + 2e-  
B)  2H+(aq) + 2e- $\rightarrow$ H2(g) 
C)  2H+(aq) + Cu(s) $\rightarrow$ H2(g) + Cu2+(aq) 
D)  Cu2+(aq) + 2e- $\rightarrow$ Cu(s) 
E)  H2(g) $\rightarrow$2H+(aq) + 2e-  
A)  Cu(s) $\rightarrow$Cu2+(aq) + 2e-  
B)  2H+(aq) + 2e- $\rightarrow$ H2(g) 
C)  2H+(aq) + Cu(s) $\rightarrow$ H2(g) + Cu2+(aq) 
D)  Cu2+(aq) + 2e- $\rightarrow$ Cu(s) 
E)  H2(g) $\rightarrow$2H+(aq) + 2e-

Calculate the solubility product of calcium hydroxide given that the solubility of Ca(OH)₂(s) in water at 25^$\circ$C is 0.011 M.

Choose the effective pH range of a HF/NaF buffer.For HF,K_a = 3.5 * 10^-⁴.

Given the half reaction: NO₃^-(aq) $\rightarrow$ NO(g),In acidic solution,How many electrons appear in the half-reaction when it is properly balanced?

The standard potential of the cell Pb(s)|PbSO₄(s)|SO₄²^-(aq)M Pb²⁺(aq)|Pb(s) Is +0.23 V at 25^$\omicron$C.Calculate the K_sp of PbSO₄.

The following 0.1 M aqueous solutions are arranged in order of increasing pH, with the highest pH on the far right. Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

What are the products of the electrolytic reduction of copper from aqueous CuSO₄?

In liquid ammonia,the acid HB is a strong acid if it is a weaker proton donor than NH₄⁺.

A solution is prepared by mixing equal volumes of 0.40 M HF(aq)with 0.40 M KOH(aq).This solution is a buffer.

You have available the following reagents as 0.10 M aqueous solutions: NaOH, HCl,HCN (pK_a = 9.31),Aniline (pK_b = 9.13),HNO₂ (pK_a = 3.25),And CH₃NH₂ (pK_b = 3.34).Which two reagents would you use to make a buffer with a pH of 10.6?

The pH of 0.010 M H₃PO₄(aq) is 2.24.Estimate the concentration of HPO₄²^- in the solution.For H₃PO₄,The values of K_a1,K_a2,And K_a3 are 7.6 * 10^-³,6.2 * 10^-⁸,And 2.1 * 10^-¹³,Respectively.

Estimate the pH of 0.10 M Na₂HPO₄(aq) given pK_a1 = 2.12, PK_a2 = 7.21,And pK_a3 = 12.68 for phosphoric acid.

Calculate the [OH^-] in an aqueous solution that is 0.125 M NH₃ and 0.300 M NH₄Cl .The value of K_b for NH₃ is 1.8 * 10^-⁵.

The K_a of phenol is 1.3 * 10^-¹⁰ .For a solution labeled "1.0 * 10^-³ M aqueous phenol,"

What is the equilibrium constant for the titration reaction involving CH₃NH₂(aq) and HBr(aq)?

If equal volumes of 0.004 M Pb(NO₃)₂(aq) and 0.004 M KI(aq) Are mixed,What reaction,If any,Occurs? The value of K_sp for PbI₂ is 1.4 * 10^-⁸.

Silver bromide is most soluble in

Calculate the [OH^-] in an aqueous solution that is 0.125 M NH₃ and 0.125 M NH₄Cl .The value of K_b for NH₃ is 1.8 * 10 ^-⁵.

A cell that uses bromine to oxidize hydrogen to H⁺ under standard conditions at 298 K has a negative potential?

For the cell diagram Pt|H₂(g),H⁺(aq)M Cu²⁺(aq)|Cu(s) Which reaction occurs at the anode?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

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Exam 6: Reactions

Calculate the solubility product of calcium hydroxide given that the solubility of Ca(OH)2(s) in water at 25 ∘\circ∘ C is 0.011 M.

Choose the effective pH range of a HF/NaF buffer.For HF,Ka = 3.5 * 10-4.

Given the half reaction: NO3-(aq) →\rightarrow→ NO(g),In acidic solution,How many electrons appear in the half-reaction when it is properly balanced?

The standard potential of the cell Pb(s)|PbSO4(s)|SO42-(aq)M Pb2+(aq)|Pb(s) Is +0.23 V at 25 ο\omicronο C.Calculate the Ksp of PbSO4.

The following 0.1 M aqueous solutions are arranged in order of increasing pH, with the highest pH on the far right. Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

What are the products of the electrolytic reduction of copper from aqueous CuSO4?

In liquid ammonia,the acid HB is a strong acid if it is a weaker proton donor than NH4+.

A solution is prepared by mixing equal volumes of 0.40 M HF(aq)with 0.40 M KOH(aq).This solution is a buffer.

You have available the following reagents as 0.10 M aqueous solutions: NaOH, HCl,HCN (pKa = 9.31),Aniline (pKb = 9.13),HNO2 (pKa = 3.25),And CH3NH2 (pKb = 3.34).Which two reagents would you use to make a buffer with a pH of 10.6?

The pH of 0.010 M H3PO4(aq) is 2.24.Estimate the concentration of HPO42- in the solution.For H3PO4,The values of Ka1,Ka2,And Ka3 are 7.6 * 10-3,6.2 * 10-8,And 2.1 * 10-13,Respectively.

Estimate the pH of 0.10 M Na2HPO4(aq) given pKa1 = 2.12, PKa2 = 7.21,And pKa3 = 12.68 for phosphoric acid.

Calculate the [OH-] in an aqueous solution that is 0.125 M NH3 and 0.300 M NH4Cl .The value of Kb for NH3 is 1.8 * 10-5.

The Ka of phenol is 1.3 * 10-10 .For a solution labeled "1.0 * 10-3 M aqueous phenol,"

What is the equilibrium constant for the titration reaction involving CH3NH2(aq) and HBr(aq)?

If equal volumes of 0.004 M Pb(NO3)2(aq) and 0.004 M KI(aq) Are mixed,What reaction,If any,Occurs? The value of Ksp for PbI2 is 1.4 * 10-8.

Silver bromide is most soluble in

Calculate the [OH-] in an aqueous solution that is 0.125 M NH3 and 0.125 M NH4Cl .The value of Kb for NH3 is 1.8 * 10 -5.

A cell that uses bromine to oxidize hydrogen to H+ under standard conditions at 298 K has a negative potential?

For the cell diagram Pt|H2(g),H+(aq)M Cu2+(aq)|Cu(s) Which reaction occurs at the anode?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

Calculate the solubility product of calcium hydroxide given that the solubility of Ca(OH)₂(s) in water at 25^$\circ$C is 0.011 M.

Choose the effective pH range of a HF/NaF buffer.For HF,K_a = 3.5 * 10^-⁴.

Given the half reaction: NO₃^-(aq) $\rightarrow$ NO(g),In acidic solution,How many electrons appear in the half-reaction when it is properly balanced?

The standard potential of the cell Pb(s)|PbSO₄(s)|SO₄²^-(aq)M Pb²⁺(aq)|Pb(s) Is +0.23 V at 25^$\omicron$C.Calculate the K_sp of PbSO₄.

What are the products of the electrolytic reduction of copper from aqueous CuSO₄?

In liquid ammonia,the acid HB is a strong acid if it is a weaker proton donor than NH₄⁺.

You have available the following reagents as 0.10 M aqueous solutions: NaOH, HCl,HCN (pK_a = 9.31),Aniline (pK_b = 9.13),HNO₂ (pK_a = 3.25),And CH₃NH₂ (pK_b = 3.34).Which two reagents would you use to make a buffer with a pH of 10.6?

The pH of 0.010 M H₃PO₄(aq) is 2.24.Estimate the concentration of HPO₄²^- in the solution.For H₃PO₄,The values of K_a1,K_a2,And K_a3 are 7.6 * 10^-³,6.2 * 10^-⁸,And 2.1 * 10^-¹³,Respectively.

Estimate the pH of 0.10 M Na₂HPO₄(aq) given pK_a1 = 2.12, PK_a2 = 7.21,And pK_a3 = 12.68 for phosphoric acid.

Calculate the [OH^-] in an aqueous solution that is 0.125 M NH₃ and 0.300 M NH₄Cl .The value of K_b for NH₃ is 1.8 * 10^-⁵.

The K_a of phenol is 1.3 * 10^-¹⁰ .For a solution labeled "1.0 * 10^-³ M aqueous phenol,"

What is the equilibrium constant for the titration reaction involving CH₃NH₂(aq) and HBr(aq)?

If equal volumes of 0.004 M Pb(NO₃)₂(aq) and 0.004 M KI(aq) Are mixed,What reaction,If any,Occurs? The value of K_sp for PbI₂ is 1.4 * 10^-⁸.

Calculate the [OH^-] in an aqueous solution that is 0.125 M NH₃ and 0.125 M NH₄Cl .The value of K_b for NH₃ is 1.8 * 10 ^-⁵.

A cell that uses bromine to oxidize hydrogen to H⁺ under standard conditions at 298 K has a negative potential?

For the cell diagram Pt|H₂(g),H⁺(aq)M Cu²⁺(aq)|Cu(s) Which reaction occurs at the anode?